Classify the solute represented in each of the following equations as a strong, weak, or nonelectrolyte:
b. NH₃(g) + H₂O(l) ⇌ NH₄⁺(aq) + OH^–(aq)

Verified step by step guidance

1. Identify the solute in the given equation. In this case, the solute is NH₃ (ammonia).
2. Examine the reaction provided: NH₃(g) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq). Notice the double arrow (⇌), which indicates that the reaction is reversible and does not go to completion.
3. Understand the behavior of NH₃ in water. Ammonia reacts with water to form NH₄⁺ (ammonium ion) and OH⁻ (hydroxide ion), but only a small fraction of NH₃ molecules ionize. This partial ionization is characteristic of a weak electrolyte.
4. Recall the definition of a weak electrolyte: A weak electrolyte partially ionizes in solution, producing a small number of ions while most of the solute remains in its molecular form.
5. Classify NH₃ as a weak electrolyte based on its partial ionization in water and the reversible nature of the reaction.

Key Concepts

Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. They are classified into strong electrolytes, which completely dissociate into ions, weak electrolytes, which partially dissociate, and nonelectrolytes, which do not dissociate at all. Understanding this classification is crucial for analyzing chemical reactions in aqueous solutions.

Strong vs. Weak Electrolytes

Strong electrolytes, such as sodium chloride, fully ionize in solution, resulting in a high concentration of ions. In contrast, weak electrolytes, like ammonia (NH₃), only partially ionize, leading to a lower concentration of ions. This distinction affects the conductivity of the solution and is essential for classifying solutes in chemical equations.

Ammonia in Water

When ammonia (NH₃) is dissolved in water, it acts as a weak base, partially reacting with water to form ammonium ions (NH₄⁺) and hydroxide ions (OH⁻). This equilibrium reaction indicates that ammonia is a weak electrolyte, as it does not fully dissociate into ions. Recognizing this behavior is key to classifying ammonia in the context of electrolyte strength.